COMPARATIVE BEHAVIOR STUDIES OF CINNAMIC ACID USING ISOTHERMAL AND NONISOTHERMAL KINETIC METHODS

In this work, a thermal behavior study of cinnamic acid was made using isothermal and nonisothermal kinetics methods. Thermogravimetric curves were obtained to determine the kinetic parameters of its decomposition process. Cinnamic acid was melted at T(peak) = 135.5 degrees C and the decomposition started at 160 degrees C. The obtained activation energy was 71.13 kJ/mol and 65.77 kJ/mol for isothermal and nonisothermal methods, respectively. The decomposition kinetics for both methods occurs at a constant rate, is of zero order, and is independent of the concentration of the reactants.